CHM1045 Exam 2 Review: Lectures 13–18

Practice vocabulary flashcards for CHM1045 Exam 2 covering reaction types, stoichiometry, aqueous solutions, oxidation-reduction, acid-base neutralization, limiting reactants, yields, and combustion analysis.

Synthesis Reaction

A chemical reaction where two or more simple reactants combine to form a single product, following the general pattern $A + B \rightarrow AB$.

Decomposition Reaction

A chemical reaction where a single compound breaks down into two or more simpler substances, following the general pattern $AB \rightarrow A + B$.

Single Replacement Reaction

A chemical reaction where an uncombined element replaces another element within a compound, following the general pattern $A + BC \rightarrow AC + B$.

Double Replacement Reaction

A chemical reaction where two ionic compounds swap partner ions, following the general pattern $AB + CD \rightarrow AD + CB$.

Combustion Reaction

A chemical reaction in which a fuel reacts with oxygen, producing carbon dioxide and water ($\text{Fuel} + O_2 \rightarrow CO_2 + H_2O$ for complete combustion of a $C/H/O$ compound).

Avogadro's Number

The stoichiometric conversion factor defining the number of particles contained in one mole: $6.022 \times 10^{23}\,\text{particles/mol}$.

Strong Electrolyte

A substance that completely dissociates or ionizes into ions in water, including strong acids, strong bases, and soluble ionic compounds.

Weak Electrolyte

A substance that only partially ionizes into ions in water, consisting primarily of weak acids and weak bases.

Nonelectrolyte

A substance that produces no ions when dissolved in water, typically consisting of covalent molecular compounds such as sugars, alcohols, and hydrocarbons.

Complete Ionic Equation

A chemical equation in which all dissolved aqueous strong electrolytes are written separated into their constituent individual ions with charges and states, while leaving solids, liquids, gases, and weak electrolytes intact.

Spectator Ions

Ions present in an aqueous solution that remain unchanged in both state and charge on both sides of a chemical reaction and are canceled out to write the net ionic equation.

Net Ionic Equation

A chemical equation obtained by removing spectator ions from a complete ionic equation, displaying only the species directly involved in the reaction.

Oxidation

The chemical process involving the loss of electrons, resulting in an increase in the oxidation state of the species.

Reduction

The chemical process involving the gain of electrons, resulting in a decrease in the oxidation state of the species.

Reducing Agent

The reactant that donates electrons and becomes oxidized, thereby reducing another chemical species.

Oxidizing Agent

The reactant that accepts electrons and becomes reduced, thereby oxidizing another chemical species.

Precipitate

An insoluble solid substance that separates out from solution as a product of an aqueous reaction.

Neutralization Reaction

A chemical reaction between an acid and a base, typically producing a salt and water: $\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}$.

Limiting Reactant

The reactant in a chemical reaction that is consumed first and determines the maximum theoretical amount of product that can form.

Excess Reactant

The reactant remaining unreacted after the limiting reactant has been completely consumed.

Theoretical Yield

The maximum amount of product calculated and predicted by stoichiometry to form from a given quantity of limiting reactant.

Actual Yield

The amount of product experimentally collected and measured from a chemical reaction.

Percent Yield

A measure of reaction efficiency calculated by comparing the actual yield to the theoretical yield: $\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\times100$

Combustion Analysis

An experimental technique where an unknown compound containing carbon, hydrogen, and oxygen is burned in excess $O_2$ to determine its empirical and molecular formula by measuring the collected masses of $CO_2$ and $H_2O$.